MnOz catalyst H, Oot O2 (gas) HOOH 2 Ce)' H20+ ē R electrons HQ + NHz ->

Write a balanced chemical equation based on the following description: solid cesium reacts with solid cesium nitrite to form cesium oxide and nitrogen gas.

Balance the following chemical equation. NaHCO3 + H3CgH507¬Na3C6H;07 + H20+ CO2

Balance the following chemical equations (include the states of matter)     The hydrolysis of P4O10(s) with H2O(l) to produce phosphoric acid, H3PO4(l )

21. Nitric acid is manufactured in the Oswald process, which involves the catalytic oxidation of ammonia according to the following equations: (i) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) (ii) 2 NO(g) + O2(8) 2 NO2(g); (iii) 3 NO2(g) + H2O(1) → 2 HNO3(aq) + NO(g); (NO is fed back into the second reactor) (a) The above equations may be combined to yield the following equation. Balance this equation. NH3(g) +_O2(g) + _H2O(1) _HNO3(1) + _H,O(1) + NO(g) (b) What is the mole fraction of NH3 that becomes nitric acid in one reaction cycle? (c) How many kilograms of HNO3 will be produced in one reaction cycle from 1.00 m³ of NH3, measured at STP, if the overall yield is 92.0%? (d) If concentrated nitric acid contains 70.0% (by mass) of HNO3 and the solution has density of 1.48 g/mL, how many litters of concentrated nitric acid is produced in this process at the above reaction yield? (Answers: (b) 2/3; (c) 1.73 kg of HNO3; (d) 1.67 L)